C6 Rates of Reaciton
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Last updated about 1 month ago
33 questions
4.6.1.1 Calculating rates of reaction
1
What is rate?
What is rate?
1
What reaction is most suitable to measure rate?
What reaction is most suitable to measure rate?
2
Select the correct equations for calculating rate of reaction
Select the correct equations for calculating rate of reaction
2
What are suitable units of rate?
What are suitable units of rate?
1
What is always the correct unit of time?
What is always the correct unit of time?
1
We produce 10g in 2 minutes. What is the average rate of reaction?
We produce 10g in 2 minutes. What is the average rate of reaction?
1
At the beginning of a chemical reaction, the rate is....
At the beginning of a chemical reaction, the rate is....
2
What two pieces of measuring equipment is he going to use to capture gas is this experiment?
What two pieces of measuring equipment is he going to use to capture gas is this experiment?
1
What pieces of equipment is best for measuring the volume of a liquid, like acid?
What pieces of equipment is best for measuring the volume of a liquid, like acid?
1
Which piece of equipment is he using to capture gas in the first method?
Which piece of equipment is he using to capture gas in the first method?
1
How often do you need to measure the gas produced?
How often do you need to measure the gas produced?
1
The first time he did this, he used 2 mol/dm3. The second time time he is using 1 mol/dm3. Do you think it will be faster or slower?
The first time he did this, he used 2 mol/dm3. The second time time he is using 1 mol/dm3. Do you think it will be faster or slower?
1
What piece of equipment captures the gas in this second experiment?
What piece of equipment captures the gas in this second experiment?
1
What piece of equipment measures time for all his experiments?
What piece of equipment measures time for all his experiments?
1
What do both experiments level off at the same point?
What do both experiments level off at the same point?
3
List the 3 sources of error from the video
List the 3 sources of error from the video
1
What is the volume of gas in the syringe?
Volume = _______ cm3
1
Which apparatus would measure 50cm3 of hydrochloric acid with the greatest accuracy
Which apparatus would measure 50cm3 of hydrochloric acid with the greatest accuracy
1
The student measured the volume of gas produced every 20 seconds for 2 minutes.
The volume of gas was zero at the start of the experiment.
The measured volumes of gas were: 26 cm3 38 cm3 47 cm3 55 cm3 59 cm3 60 cm3
Complete the table to show these results.
Tick one box to select the correct unit for each variable.
The student measured the volume of gas produced every 20 seconds for 2 minutes.
The volume of gas was zero at the start of the experiment.
The measured volumes of gas were: 26 cm3 38 cm3 47 cm3 55 cm3 59 cm3 60 cm3
Complete the table to show these results.
Tick one box to select the correct unit for each variable.
1
Match the method to the unit of rate of reaction
Match the method to the unit of rate of reaction
| Draggable item | arrow_right_alt | Corresponding Item |
|---|---|---|
Marble chips and hydrochloric acid are placed in a conical flask on a top-pan balance. | arrow_right_alt | g/s |
Marble chips in hydrochloric acid are placed in a conical flask, with a bung attached to a gas syringe at the opening. | arrow_right_alt | cm3/s |
A conical flask containing sodium thiosulfate and dilute hydrochloric acid is placed on a piece of paper with a cross on it. | arrow_right_alt | s |
2
Describe the trends shown in the student’s results.
1
The symbol equation for the decomposition of hydrogen peroxide (H2O2) is:
2 H2O2 → 2 H2O + O2
Complete the word equation for the decomposition of hydrogen peroxide.
hydrogen peroxide → _______ + _______
1
Measuring the gas produced, the mass lost, or the light transmitted are all ways of measuring the rate of reaction.
Measuring the gas produced, the mass lost, or the light transmitted are all ways of measuring the rate of reaction.
6
Describe to Jun a method he could use to measure rate of reaction, and an advantage of using this method.
Describe to Jun a method he could use to measure rate of reaction, and an advantage of using this method.
4.6.1.2 Factors affecting rate of Reaction
1
Increasing the pressure of gases in a reaction will increase the rate of reaction.
Increasing the pressure of gases in a reaction will increase the rate of reaction.
1
Increasing the temperature of reactants increases the number of particles in the reaction.
Increasing the temperature of reactants increases the number of particles in the reaction.
1
There are five main factors that affect the rate of reaction.
There are five main factors that affect the rate of reaction.
1
For every 10°C temperature increase, the rate of reaction triples.
For every 10°C temperature increase, the rate of reaction triples.
4.6.1.3 Collision theory and activation energy
1
Collision theory states that particles must collide with enough energy in order to react.
Collision theory states that particles must collide with enough energy in order to react.
1
The minimum amount of energy required for a successful collision is called the starter energy.
The minimum amount of energy required for a successful collision is called the starter energy.
4.6.1.4 Catalysts
1
Different catalysts are needed for different reactions.
Different catalysts are needed for different reactions.
1
During a reaction, a catalyst gets used up and has to be replaced each time.
During a reaction, a catalyst gets used up and has to be replaced each time.
1
Catalysts are usually cheap transition metals.
Catalysts are usually cheap transition metals.
4.6.2 Reversible reactions and dynamic equilibrium